Chemistry:Magnesium chlorate

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Magnesium chlorate
Mg(aq6(ClO3)2.svg
Names
IUPAC name
Magnesium dichlorate hexahydrate
Systematic IUPAC name
Magnesium dichlorate
Other names
  • Magnesium(II) chlorate
Identifiers
3D model (JSmol)
ChemSpider
EC Number
  • 233-711-1
UNII
UN number 2723
Properties
Mg(ClO3)2
Molar mass 191.20 g/mol
Appearance White crystalline solid
Density 1.747 g/cm3 (hexahydrate)[1]
Melting point 35 °C (95 °F; 308 K)[2]
Boiling point 120 °C (248 °F; 393 K)[2] (decomposition)
114 g/100 ml (0 °C)
123 g/100 ml (10 °C)
135 g/100 ml (20 °C)
155 g/100 ml (30 °C)
178 g/100 ml (50 °C)
242 g/100 ml (60 °C)
268 g/100 ml (100 °C)[2]
Solubility in acetone Soluble
Structure[1]
Monoclinic
P21/c
a = 6.39 Å, b = 6.51 Å, c = 13.90 Å
α = 90°, β = 100.3°, γ = 90°
590.1 Å3
Hazards
GHS pictograms GHS07: Harmful
GHS Signal word Warning
H302, H332
Lethal dose or concentration (LD, LC):
6348 mg/kg (rat, oral)
Related compounds
Other cations
Calcium chlorate
Strontium chlorate
Barium chlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Magnesium chlorate refers to inorganic compounds with the chemical formula Mg(ClO3)2(H2O)x. The anhydrous (x = 0), dihydrate (x = 2), and hexahydrate (x = 6) are known. These are thermally labile white solids. The hexahydrate has been identified on the Martian surface.[3]

Production

Samples of magnesium chlorate were first claimed in 1920 as the result of treating magnesium oxide with chlorine. A more modern method involves electrolysis of magnesium chloride.[4] The magnesium chlorate can be purified by exploiting its solubility in acetone.[4]

Properties

The hexahydrate Mg(ClO3)2·6H2O decomposes to the tetrahydrate at 35 °C. At 65 °C, it dehydrates to the dihydrate, then at 80 °C forms a basic salt. If further heated to 120 °C it decomposes to water, oxygen, chlorine, and magnesium oxide.[2]

As confirmed by X-ray crystallography, the di- and hexahydrates feature octahedral Mg2+ centers. The other ligands are water, exclusively in the hexahydrate. In the dihydrate, chlorate is also coordinated and functions as a bridging ligand.[1]

Uses

Magnesium(II) chlorate is used as a powerful desiccant and a defoliant for cotton, potato, and rice. It is also found as a lubricant in eye drops as an inactive ingredient.[5]

Hazards

Magnesium chlorate is an oxidizer and can in principle form explosive mixtures.

References

  1. 1.0 1.1 1.2 Kossev, K; Tsvetanova, L.; Dimowa, L.; Nikolova, R.; Shivachev, B. (2013). "Synthesis and Crystal Structure of Magnesium Chlorate Dihydrate and Magnesium Chlorate Hexahydrate". Bulgarian Chemical Communications 45: 543–548. 
  2. 2.0 2.1 2.2 2.3 Joseph William Mellor (1922). Supplement to Mellor's Comprehensive Treatise on Inorganic and Theoretical Chemistry: suppl. 3. K, Rb, Cs, Fr. Longmans, Green and Company. 
  3. Ojha, Lujendra; Wilhelm, Mary Beth; Murchie, Scott L.; McEwen, Alfred S.; Wray, James J.; Hanley, Jennifer; Massé, Marion; Chojnacki, Matt (2015). "Spectral evidence for hydrated salts in recurring slope lineae on Mars". Nature Geoscience 8 (11): 829–832. doi:10.1038/ngeo2546. Bibcode2015NatGe...8..829O. 
  4. 4.0 4.1 Herbert Maxim (1948) (in English). The electrolytic production of magnesium chlorate and perchlorate. the Department of Chemical Engineering: University of Southern California. 
  5. "MAGNESIUM CHLORATE" (in English). U.S. Department of Health & Human Services. https://drugs.ncats.io/substance/M536P01U3N#general.